A molecule has an empirical formula of ch, and its molar mass is known to be 26 g/mol and the molecular formula is C₂H₂ ethyne
Molecular formula of compound is (CH)n and the given molar mass is 26g/mol
Molar mass of (CH)n, C=12=n(12+1)=13n
So 13n and n=2
=13×2=26 and given molar mass is also 26g/mol
So here two carbon and two hydrogen so molecular formula is C₂H₂ and name is ethyne
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Answer: Thus 0.724 mol of 
are needed to obtain 18.6 g of 
Explanation:
To calculate the moles :
According to stoichiometry :
2 moles of are produced by = 1 mole of
Thus 1.09 moles of will be produced by =
of
But as yield of reaction is 75.6 %, the amount of needed is =
Thus 0.724 mol of are needed to obtain 18.6 g of
The answer would be the third option. (the angle at which the light hits the surface.)<span>
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Answer:
The play will be more appealing to a younger audience.
Explanation:
A younger audience will more likely appreciate current pop hits rather than classical score.
Answer : The partial pressure of 
and 
is, 216.5 mmHg and 649.5 mmHg
Explanation :
According to the Dalton's Law, the partial pressure exerted by component 'i' in a gas mixture is equal to the product of the mole fraction of the component and the total pressure.
Formula used :
So,
where,
= partial pressure of gas
= mole fraction of gas
= total pressure of gas
= moles of gas
= total moles of gas
The balanced decomposition of ammonia reaction will be:
Now we have to determine the partial pressure of and
Given:
and,
Given:
Thus, the partial pressure of and is, 216.5 mmHg and 649.5 mmHg
