Problem: For each reaction, calculate the mass (in grams) of the product formed when 10.5 g of the underlined reactant completely reacts.Assume that there is more than enough of the other reactant.Part A2K(s)+ Cl2(g) →2KCl(s)Part B2K(s)+ Br2(l) →2KBr(s)Part C4Cr(s)+ 3O2(g) →2Cr2O3(s)Part D2Sr(s) + O2(g)→2SrO(s)

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Assume that there is more than enough of the other reactant.

Part A:

2 K(s) + Cl2(g) → 2 KCl(s)

mass Cl2 = 10.5 g
molar mass of Cl2 = 70.90 g/mol
molar mass of KCl = 74.55 g/mol
mole-to-mole comparison: 1 mol Cl2 forms 2 mol KCl

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Problem Details

For each reaction, calculate the mass (in grams) of the product formed when 10.5 g of the underlined reactant completely reacts.

Assume that there is more than enough of the other reactant.

Part A

2K(s)+ Cl2(g) →2KCl(s)

Part B

2K(s)+ Br2(l) →2KBr(s)

Part C

4Cr(s)+ 3O2(g) →2Cr2O3(s)

Part D

2Sr(s) + O2(g)→2SrO(s)

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