I want to see if i got my answer correct for #1 but I need help on #2
1.A 150g aluminum pan containing 500g of water is heated on a stove for 5 minutes. The temperature goes from 23.5C to 48.9C. How much heat was absorbed. (s for Al is .900j/g C, s for H2O is 4.184 j/g C) I got 3429J AL and 53136.8J H2O heat absorbed?
2. When a 1.000 g sample of the rocket fuel hydrazine, N2H4, is burned in a bomb calorimeter which contains 1200g of water, the temperature rises from 24.62C to 28.16C. If the C for the bomb is 840 J/C
Calculate: q reaction for combustion of a one-gram sample
and
q reaction for combustion of one mole of hydrazine in the bomb calorimeter
To solve problem #2, we need to calculate the amount of heat absorbed during the combustion of a 1.000 g sample of hydrazine and the combustion of one mole of hydrazine.
1. To find the heat absorbed during the combustion of a 1.000 g sample of hydrazine, we can use the formula:
q = m * C * ΔT
where:
q = heat absorbed
m = mass of the substance (in this case, 1.000 g)
C = specific heat capacity of water (4.184 J/g°C)
ΔT = change in temperature (in this case, 28.16°C - 24.62°C)
Using the formula, we can calculate:
q = 1.000 g * 4.184 J/g°C * (28.16°C - 24.62°C)
Simplifying the equation:
q = 1.000 g * 4.184 J/g°C * 3.54°C
Calculating further:
q = 14.77 J
Therefore, the heat absorbed during the combustion of a 1.000 g sample of hydrazine is 14.77 J.
2. To find the heat absorbed during the combustion of one mole of hydrazine, we need to calculate the molar mass of hydrazine (N2H4) and convert mass to moles.
The molar mass of N2H4 is:
2(N) + 4(H) = 2(14.01 g/mol) + 4(1.01 g/mol) = 28.02 g/mol + 4.04 g/mol = 32.06 g/mol
To convert the mass of 1.000 g of hydrazine to moles, we use the equation:
moles = mass / molar mass
moles = 1.000 g / 32.06 g/mol
Calculating further:
moles ≈ 0.0312 mol
Now, to find the heat absorbed during the combustion of one mole of hydrazine, we multiply the heat absorbed during the combustion of a 1.000 g sample (14.77 J) by the number of moles:
q = (14.77 J) * (0.0312 mol)
Calculating further:
q ≈ 0.4615 J/mol
Therefore, the heat absorbed during the combustion of one mole of hydrazine in the bomb calorimeter is approximately 0.4615 J/mol.