1.) Gaseous hydrogen and oxygen can be prepared in the laboratory from the decom

Question

1.) Gaseous hydrogen and oxygen can be prepared in the laboratory from the decomposition of gaseous water. The equation for the reaction is

2H2O(g)====>2H2(g)+O2(g)

Calculate how many grams of O2(g) can be produced from 85.6 grams of H2O(g).

2.) For the following chemical reaction, how many moles of potassium phosphate will be produced from 41.8 g of potassium hydroxide?

3KOH+H3PO4====>K3PO4+3H2O

3.) Balance the following combustion reaction in order to answer the following questions. Use lowest whole-number coefficients.

C2H4+O2====>CO2+H2O

You are given 3.0 moles of O2 to react with 1.20 × 102 g C2H4. Upon completion of the reaction, will there be any remaining C2H4?

a. yes, there will still be C2H4 remaining

b. no, all C2H4 will be used up in the reaction

Explanation / Answer

1)

mass of H2O = 85.6 g

molar mass of H2O = 18.0 g/mol

mol of H2O = (mass)/(molar mass)

= 85.6/18.0

= 4.76 mol

Balanced chemical equation is:

2H2O(g)====>2H2(g)+O2(g)

According to balanced equation

mol of H2 formed = (2/2)* moles of H2O

= (2/2)*4.76

= 4.76 mol

masss of H2 = number of mol * molar mass

= 4.76*2.0

= 9.51 g

Answer: 9.51 g

i am allowed to answer only 1 question at a time

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