Answer:
4.5L of gas are produced
Explanation:
Based on the reaction:
Zn + H2SO4 → ZnSO4 + H2(g)
<em>Where 1 mole of Zn reacts with 1 mole of sulfuric acid to produce 1 mole of H2, the gas</em>
<em />
To solve this question we must find the moles of each reactant in order to find limiting reactant and, thus, the moles of H2 produced. Then using PV=nRT we can find the volume of the gas:
<em>Moles Zn -Molar mass: 65.38g/mol-</em>
13g * (1mol / 65.38g) = 0.20 moles Zn
<em>Moles H2SO4 -Molar mass: 98g/mol-</em>
400g * 10% = 40g H2SO4 * (1mol / 98g) = 0.41 moles H2SO4
As the ratio of the reaction is 1:1, the limiting reactant is Zn and the moles produced of H2 are 0.20 moles
Using PV = nRT; V = nRT/ P
<em>Where V is the volume of the gas </em>
<em>n are the moles = 0.20 moles</em>
<em>R is gas constant = 0.082atmL/molK</em>
<em>T is absolute temperature = 273.15K at STP</em>
<em>P is pressure = 1atm at STP</em>
<em />
V = 0.20mol*0.082atmL/molK*273.15K / 1atm
V = 4.5L of gas are produced
<em />
