2 years ago

How much energy is released during the formation of 1 mol H2O

Chemistry

1 answer:

kari74 [83]2 years ago

7 0

2.81 moles NO

I HOPE THAT RIGHT

You might be interested in

A stock solution of 1.00 M Fe2(SO4)3 is available. How many milliliters are

Andrews [41]

Answer:

375 mL

Explanation:

M1*V1 = M2*V2

M1 = 1.00 M

V1 = ?

M2 = 0.750 M

V2 = 0.500 L

1.00 M * V1 = 0.750 M * 0.500 L

V1 = 0.750*0.500/1.00 = 0.375 L = 375 mL

5 0

3 years ago

During _____________ there are 24 hours of daylight at the North Pole.

Tresset [83]

Answer:

summer

The North Pole stays in full sunlight all day long throughout the entire summer (unless there are clouds)

8 0

2 years ago

1. Chlorobenzene, C6H5C1, is used in the production of chemicals such as aspirin

Natalka [10]

C6H6(l) + 6 Cl2(g) = C6Cl6(s) + 6 HCl(g)

3 0

2 years ago

the heat of fusion of acetone is 5.7 kJ/mol. Calculate to two significant figures the entropy change when 6.3 mol of acetone mel

shtirl [24]

<u>Answer:</u> The entropy change of the process is $2.0\times 10^2J/K$

<u>Explanation:</u>

To calculate the entropy change for different phase at same temperature, we use the equation:

$\Delta S=n\times \frac{\Delta H_{f}}{T}$

where,

$\Delta S$ = Entropy change

n = moles of acetone = 6.3 moles

$\Delta H_{f}$ = enthalpy of fusion = 5.7 kJ/mol = 5700 J/mol (Conversion factor: 1 kJ = 1000 J)

T = temperature of the system = $-94.7^oC=[273-94.7]=178.3K$

Putting values in above equation, we get:

$\Delta S=\frac{6.3mol\times 5700J/mol}{178.3K}\\\\\Delta S=201.4J/K=2.0\times 10^2J/K$

Hence, the entropy change of the process is $2.0\times 10^2J/K$

4 0

3 years ago

A reaction that absorbs energy

coldgirl [10]

Answer:

Endothermic Reaction

Explanation:

5 0

2 years ago

Read 2 more answers