(5 pts) Calculating Heat from Thermochemical Equations

Chemistry

1 answer:

Vadim26 [7]2 years ago

8 0

The heat that is released by the combustion of 3.5 moles of methane is 3115 kJ/mol.

<h3>What is a thermochemical equation?</h3>

A thermochemical equation is a reaction equation that incorporates the amount of heat lost/gained.

In this case, the reaction equation is; CH4 + O2 ----->CO2 + 2H2O dH = -890 kJ/mol

If 1 mole of methane releases 890 kJ/mol

3.5 moles of methane will release 3.5 moles * 890 kJ/mol/1 mole

= 3115 kJ/mol

Learn more about combustion reaction:brainly.com/question/12172040?

#SPJ1

You might be interested in

The percent yield of a chemical reaction is

Veronika [31]

Answer:

the measured amount of product that is made from a given amount of reactant

Explanation:

google & quizlet

4 0

2 years ago

Read 2 more answers

What color would litmus paper turn in a solution of baking soda? Explain your answer in terms of pH.

madam [21]

Blue

When red litmus paper comes into contact with any alkaline substance, it turns blue. Some examples of alkaline substances are ammonia gas, milk of magnesia, baking soda and limewater.

3 0

2 years ago

A frictionless piston cylinder device is subjected to 1.013 bar external pressure. The piston mass is 200 kg, it has an area of

Bad White [126]

Answer:

a) $T_{2} = 360.955\,K$ , $P_{2} = 138569.171\,Pa\,(1.386\,bar)$ , b) $T_{2} = 347.348\,K$ , $V_{2} = 0.14\,m^{3}$

Explanation:

a) The ideal gas is experimenting an isocoric process and the following relationship is used:

$\frac{T_{1}}{P_{1}} = \frac{T_{2}}{P_{2}}$

Final temperature is cleared from this expression:

$Q = n\cdot \bar c_{v}\cdot (T_{2}-T_{1})$

$T_{2} = T_{1} + \frac{Q}{n\cdot \bar c_{v}}$

The number of moles of the ideal gas is:

$n = \frac{P_{1}\cdot V_{1}}{R_{u}\cdot T_{1}}$

$n = \frac{\left(101,325\,Pa + \frac{(200\,kg)\cdot (9.807\,\frac{m}{s^{2}} )}{0.15\,m^{2}} \right)\cdot (0.12\,m^{3})}{(8.314\,\frac{Pa\cdot m^{3}}{mol\cdot K} )\cdot (298\,K)}$