Question

If 5.000 g of C6H6 is burned and the heat produced from the burning is added to 5691 g of water at 21 °C, what is the final temperature of the water?

Answer #1

The balanced combustion reaction for C6H6 is
2C6H6(l)+15O2(g)⟶12CO2(g)+6H2O(l)+6542 kJ If 7.700 g C6H6 is burned
and the heat produced from the burning is added to 5691 g of water
at 21 ∘ C, what is the final temperature of the water?

When one mole of C6H6 is burned, 3.27 MJ of heat is produced.
When the heat from burning 7.19 g of C6H6 is added to 5.69 kg of
water at 21.0°C, what is the final temperature of the water?

The following equation is the balanced combustion reaction for
C6H6:
2C6H6(l)+15O2(g) = 12CO2(g)+6H2O(l)+6542KJ
If 7.800 g of C6H6 is burned and the heat produced from the
burning is added to 5691 g of water at 21 °C, what is the final
temperature of the water?

The following equation is the balanced combustion reaction for
C6H6:
2C6H6(l) + 15O2(g) ------>
12CO2(g)+6H2O(l)+6542 kJ
If 6.900 g of C6H6 is burned and the heat produced from the
burning is added to 5691 g of water at 21 °C, what is the final
temperature of the water?
please answer this is due today thank you

The following equation is the balanced combustion reaction for
C6H6:
2C6H6 (l) + 15O2 (g) --> 12CO2(g) + 6H2O(l)+6542KJ
If 8.800 g of C6H6 is burned and the heat produced from the
burning is added to 5691 g of water at 21 Celcius, what is the
final temp of the water? (in celcius)

When one mole of C 6 H 6 is burned, 3.27 MJ of heat is produced.
When the heat from burning 7.89 g of C 6 H 6 is added to 5.69 kg of
water at 21.0 ∘ C , what is the final temperature of the water? T
final =

4.05 g of methane is burned and all of the heat is from this is
absorbed by 1.0x10^3 g of 20.0 degree C water (which has a specific
heat of 4.18Jg^-1 C^-1). What is the final temperature of the
water?

A 2.50 mol sample of benzene (C6H6, 78.11 g/mol) was burned in a
bomb calorimeter with a heat capacity of 800 J/°C. The calorimeter
contained 100g of water (4.18J/g°C) and the temperature increased
by 4°C. What is the molar enthalpy of combustion for this
compound?

A 1.000g sample of benzene (C6H6) is
burned in a bomb calorimeter whose total heat capacity is 4.957 kJ/
oC. If the temperature of the calorimeter increases from
25.30 to 33.74 oC , what is the heat of combustion of
the benzene per mole.
Explanation please.

0.9410 g of phenol (C6H5OH) are burned in a bomb calorimeter
with a heat capacity of 4.630 kJ/C . The temperature of the
calorimeter increases by 6.590C. What is the heat of combustion
(Hrxn for the process of burning) of phenol?
a. -30.51 kJ/C
b. -267.5 kJ/C
c. -3051 kJ/mol
d. none of these

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