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Balance each of the following chemical equations.

b. Fe2O3(s) + HNO3(aq) → Fe(NO3)3(aq) + H2O(l)

 

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Balance each of the following chemical equations.

a. KO2(s) + H2O(l) → KOH(aq) + O2(g) + H2O2(aq)

 

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Balance the following equations:

c. AgNO3(aq) + H2SO4(aq) → Ag2SO4(s) + HNO3(aq)

 

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Balance the following equations:

b. Al(OH)3(s) + HCl(aq) → AlCl3(aq) + H2O(l)

 

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Balance the following equations:

a. Ca(OH)2(aq) + H3PO4(aq) → H2O(l) + Ca3(PO4)2(s)

 

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A common demonstration in chemistry courses involves adding  a tiny speck of manganese(IV) oxide to a concentrated hydrogen peroxide (H2O2) solution. Hydrogen peroxide decomposes quite spectacularly under these conditions to produce oxygen gas and steam (water vapor). Manganese(IV) oxide is a catalyst for the decomposition of hydrogen peroxide and is not consumed in the reaction. Write the balanced equation for the decomposition reaction of hydrogen peroxide.

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Give the balanced equation for each of the following.

d. Aqueous strontium hydroxide reacts with aqueous hydrobromic acid to produce water and aqueous strontium bromide. 

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Give the balanced equation for each of the following.

c. Solid zinc reacts with aqueous HCl to form aqueous zinc chloride and hydrogen gas.

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Give the balanced equation for each of the following.

b. Aqueous solutions of lead(II) nitrate and sodium phosphate are mixed, resulting in the precipitate formation of lead(II) phosphate with aqueous sodium nitrate as the other product.

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Give the balanced equation for each of the following.

a. The combustion of ethanol (C2H5OH) forms carbon dioxide and water vapor. A combustion reaction refers to a reaction of a substance with oxygen gas.

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A compound contains only carbon, hydrogen, and oxygen. Combustion of 10.68 mg of the compound yields 16.01 mg CO2 and 4.37 mg H2O. The molar mass of the compound is 176.1 g/mol. What are the empirical and molecular formulas of the compound?

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Maleic acid is an organic compound composed of 41.39% C, 3.47% H, and the rest oxygen. If 0.129 mol of maleic acid has a mass of 15.0 g, what are the empirical and molecular formulas of maleic acid?

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Determine the molecular formula of a compound that contains 26.7% P, 12.1% N, and 61.2% Cl, and has a molar mass of 580 g/mol.

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There are two binary compounds of mercury and oxygen. Heating either of them results in the decomposition of the compound, with oxygen gas escaping into the atmosphere while leaving a residue of pure mercury. Heating 0.6498 g of one of the compounds leaves a residue of 0.6018 g. Heating 0.4172 g of the other compound results in a mass loss of 0.016 g. Determine the empirical formula of each compound.

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The most common form of nylon (nylon-6) is 63.68% carbon, 12.38% nitrogen, 9.80% hydrogen, and 14.14% oxygen. Calculate the empirical formula for nylon-6.

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Determine the molecular formulas to which the following empirical formulas and molar masses pertain.

d. SN (184.32 g/mol)

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Determine the molecular formulas to which the following empirical formulas and molar masses pertain.

c. CoC4O4 (341.94 g/mol)

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Determine the molecular formulas to which the following empirical formulas and molar masses pertain.

b. NPCl 2 (347.64 g/mol)

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Determine the molecular formulas to which the following empirical formulas and molar masses pertain.

a. SNH (188.35 g/mol)

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Give the empirical formula for each of the compounds represented below.

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Give the empirical formula for each of the compounds represented below.

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Give the empirical formula for each of the compounds represented below.

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Give the empirical formula for each of the compounds represented below.

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Express the composition of each of the following compounds as the mass percents of its elements.

c. acetic acid, HC2H3O2

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Express the composition of each of the following compounds as the mass percents of its elements.

b. glucose, C6H12O6

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