<span>You will use an ideal gas equation here. Let us denote 'x' as the unknown sample of zinc if another 1 ml of it is added to make a total of 476mL gas. The ideal gas equation is PV = nRT. Assume atmospheric conditions and then substitute everything to the equation.
(1atm)(0.476L) = (1.85 + x)(0.08206 L-atm/mol-K)(20.5+273K)
x = 1.83 g of zinc</span>
<u>Answer:</u> The concentration of solute is 0.503 mol/L
<u>Explanation:</u>
To calculate the concentration of solute, we use the equation for osmotic pressure, which is:
where,
= osmotic pressure of the solution = 24 atm
i = Van't hoff factor = 2 (for NaCl)
c = concentration of solute = ?
R = Gas constant = 
T = temperature of the solution = ![25^oC=[273+25]=298K](https://tex.z-dn.net/?f=25%5EoC%3D%5B273%2B25%5D%3D298K)
Putting values in above equation, we get:
Hence, the concentration of solute is 0.503 mol/L
The number of moles of oxygen (O2) required to completely react with 27.4 mol of H2 is 13.7 moles.
<h3>How to calculate number of moles?</h3>
The number of moles of a substance can be calculated using stoichiometry as follows:
The following balanced chemical equation is given as follows:
2H2 + O2 = 2H2O
According to this question, 2 moles of hydrogen gas (H2) reacts with 1 mole of oxygen gas (O2).
This means that 27.4 moles of hydrogen gas (H2) will react with 27.4/2 = 13.7moles of oxygen gas.
Therefore, the number of moles of oxygen (O2) required to completely react with 27.4 mol of H2 is 13.7 moles.
Learn more about number of moles at: brainly.com/question/14919968
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Answer:
2 double bonds 2 single bonds
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