Answer: Mass of zinc that reacts with 4.11 g of hydrochloric acid to form 9.1 g of zinc chloride and 3.97 g of hydrogen gas is 8.96 g
Explanation:
According to the law of conservation of mass, mass can neither be created nor be destroyed. Thus the mass of products has to be equal to the mass of reactants. The number of atoms of each element has to be same on reactant and product side. Thus chemical equations are balanced.
Given: mass of hydrochloric acid = 4.11 g
Mass of products = Mass of zinc chloride + mass of hydrogen = 9.1 g + 3.97 g = 13.07 g
As mass of reactant = mass of products
mass of hydrochloric acid + mass of zinc = Mass of zinc chloride + mass of hydrogen
4.11 g + mass of zinc = 13.07 g
mass of zinc = 8.96 g
Answer:
3.69 g
Explanation:
Given that:
The mass m = 325 g
The change in temperature ΔT = ( 1540 - 165)° C
= 1375 ° C
Heat capacity 
= 0.490 J/g°C
The amount of heat required:
q = mcΔT
q = 325 × 0.490 × 1375
q = 218968.75 J
q = 218.97 kJ
The equation for the reaction is expressed as:
Then,
1 mole of the ethyne is equal to 26 g of ethyne required for 1544 kJ heat.
Thus, for 218.97 kJ, the amount of ethyne gas required will be:
= 3.69 g
2C6H14 + 13O2 ---> 6CO2 +14H2O
M(C6H14)=12.011*6 +1.008*14 ≈ 86.17 g/mol
86.17 g C6H14 is 1 mole.
2C6H14 + 13O2 ---> 6CO2 +14H2O
from reaction 2 mol 6 mol
from the problem 1 mol 3 mol
M(CO2)= 12.011 + 2*15.999= 44.009 g/mol
3 mol CO2*44.009 g/1 mol CO2 ≈ 132.0 g CO2
Answer : 132.0 g CO2
Explanation:
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