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3 years ago

1. Which occurs when the forward and reverse reactions occur at the same rate?

Chemistry

2 answers:

Kay [80]3 years ago

6 0

Answer:

the object will not move and remain at a state of rest

Vika [28.1K]3 years ago

5 0

Answer:

The system is in equilibrium.

Explanation:

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How much energy is required to heat 87.1 g acetone (molar mass=58.08 g/mol) from a solid at -154.0°C to a liquid at -42.0°C? The

WARRIOR [948]

Answer:

The answer to the question above is

The energy required to heat 87.1 g acetone from a solid at -154.0°C to a liquid at -42.0°C = 29.36 kJ

Explanation:

The given variables are

ΔHfus = 7.27 kJ/mol

Cliq = 2.16 J/g°C

Cgas = 1.29 J/g°C

Csol = 1.65 J/g°C

Tmelting = -95.0°C.

Initial temperature = -154.0°C

Final temperature = -42.0°C?

Mass of acetone = 87.1 g

Molar mass of acetone = 58.08 g/mol

Solution

Heat required to raise the temperature of solid acetone from -154 °C to -95 °C or 59 °C is given by

H = mCsolT = 87.1 g* 1.65 J/g°C* 59 °C = 8479.185 J

Heat required to melt the acetone at -95 °C = ΔHfus*number of moles =

But number of moles = mass÷(molar mass) = 87.1÷58.08 = 1.5

Heat required to melt the acetone at -95 °C =1.5 moles*7.27 kJ/mol = 10.905 kJ

The heat required to raise the temperature to -42 degrees is

H = m*Cliq*T = 87.1 g* 2.16 J/g°C * 53 °C = 9971.21 J

Total heat = 9971.21 J + 10.905 kJ + 8479.185 J = 29355.393 J = 29.36 kJ

The energy required to heat 87.1 g acetone from a solid at -154.0°C to a liquid at -42.0°C is 29.36 kJ

4 0

4 years ago

A bomb calorimeter has a heat capacity of 675 J/°C and contains 925 g of water. If the combustion of 0.500 mole of a hydrocarbon

ikadub [295]

<u>Answer:</u> The enthalpy of the reaction is 269.4 kJ/mol

<u>Explanation:</u>

To calculate the heat absorbed by the calorimeter, we use the equation:

$q_1=c\Delta T$

where,

q = heat absorbed

c = heat capacity of calorimeter = 675 J/°C

$\Delta T$ = change in temperature = $T_2-T_1=(53.88-24.26)^oC=29.62^oC$

Putting values in above equation, we get:

$q_1=675J/^oC\times 29.62^oC=19993.5J$

To calculate the heat absorbed by water, we use the equation:

$q_2=mc\Delta T$

where,

q = heat absorbed

m = mass of water = 925 g

c = heat capacity of water = 4.186 J/g°C

$\Delta T$ = change in temperature = $T_2-T_1=(53.88-24.26)^oC=29.62^oC$

Putting values in above equation, we get:

$q_2=925g\times 4.186J/g^oC\times 29.62^oC=114690.12J$

Total heat absorbed = $q_1+q_2$

Total heat absorbed = $[19993.5+114690.12]J=134683.62J=134.7kJ$

To calculate the enthalpy change of the reaction, we use the equation:

$\Delta H_{rxn}=\frac{q}{n}$

where,

q = amount of heat absorbed = 134.7 kJ

n = number of moles of hydrocarbon = 0.500 moles

$\Delta H_{rxn}$ = enthalpy change of the reaction

Putting values in above equation, we get:

$\Delta H_{rxn}=\frac{134.7kJ}{0.500mol}=269.4kJ/mol$

Hence, the enthalpy of the reaction is 269.4 kJ/mol

6 0

4 years ago

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Alja [10]

The answer is exposure to sunlight

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3 years ago

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Doss [256]

Answer:

filtration

Explanation:

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4 years ago

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bonufazy [111]

Aldehydes oxidise to form carboxylic acids

7 0

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