2 years ago

How many moles of neon occupy a volume of 14.3 l at stp?

1 answer:

4 0

Answer: 0.638 moles

Explanation: A total of 0.638 moles of neon are needed to occupy a volume of 14.3 L at standard temperature and pressure (STP).

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SashulF [63]

Its A because I did it on connexus

5 0

3 years ago

Dennis_Churaev [7]

Molar mass NaCl = 58 g

Mass of solute = 29 g

number of moles: mass of solute / molar mass

n = 29 / 58

n = 0.5 moles

hope this helps!

4 0

3 years ago

inn [45]

Answer:

Optically Transparent

7 0

3 years ago

kari74 [83]

Answer: 72.4 kJ/mol

Explanation:

The balanced chemical reaction is,

$C_3H_8(g)+5O_2(g)\rightarrow 3CO_2(g)+4H_2O(l)$ $\Delta H=-2220.1kJ/mol$

The expression for enthalpy change is,

$\Delta H=\sum [n\times \Delta H_f(product)]-\sum [n\times \Delta H_f(reactant)]$

$\Delta H=[(n_{CO_2}\times \Delta H_{CO_2})+(n_{H_2O}\times \Delta H_{H_2O})]-[(n_{O_2}\times \Delta H_{O_2})+(n_{C_3H_8}\times \Delta H_{C_3H_8})]$

where,

n = number of moles

$\Delta H_{O_2}=0$ (as heat of formation of substances in their standard state is zero

Now put all the given values in this expression, we get

$-2220.1=[(3\times -393.5)+(4\times -241.8)]-[(5\times 0)+(1\times \Delta H_{C_3H_8})]$

$\Delta H_{C_3H_8}=72.4kJ/mol$

Therefore, the heat of formation of propane is 72.4 kJ/mol

7 0

2 years ago

Nataly [62]

A or b I think it’s b

5 0

2 years ago