Answer : The mass of nickel(II) nitrate is, 0.4568 grams
Explanation : Given,
Molar mass of nickel(II) nitrate = 182.71 g/mole
Volume of solution = 25.0 ml
Molarity = 0.100 M
Molarity : It is defined as the mass of solute present in one liter of solution.
Formula used :
where,
w = mass of nickel(II) nitrate
M = molar mass of nickel(II) nitrate
V = volume of solution
Now put all the given values in the above formula, we get:
Therefore, the mass of nickel(II) nitrate is, 0.4568 grams
Answer:
Explanation:
<u>Calculation of the mass of chromium as:- </u>
Moles = 1.002 moles
Molar mass of chromium = 51.9961 g/mol
The formula for the calculation of moles is shown below:
Thus,
<u>Calculation of the mass of neon as:- </u>
Moles = moles
Molar mass of neon = 20.1797 g/mol
Thus,
Answer:
Explanation:
Hello,
In this case, given that the mass of the product is 0.534 g, we can infer that the percent composition of tin is:
Therefore, the percent composition of oxygen is 6.4% for a 100% in total. Thus, with such percents we compute the moles of each element in the oxide:
In such a way, for finding the smallest whole number we divide the moles of both tin and oxygen by the moles of oxygen as the smallest moles:
Therefore, the empirical formula is:
Best regards.
Answer:
Total pressure = 0,806 atm
Partial pressure of CH₄: 0,037 atm
Partial pressure of Cl₂: 0,396 atm
Partial pressure of CH₃Cl: 0,125 atm
Partial pressure of HCl: 0,125 atm
Partial pressure of Cl⁻: 0,125 atm
Explanation:
For the reaction:
2CH₄(g)+3Cl₂(g)⟶2CH₃Cl(g)+2HCl(g)+2Cl⁻(g)
295 mL≡ 0,295L of methane at STP are:
n = PV/RT
P = 1 atm; V = 0,295L; R = 0,082atmL/molK; T = 273K.
moles of methane: 0,0132 moles
For 725 mL of chlorine ≡ 0,725L
moles of chlorine at STP are: ≡ 0,0324 moles
For a complete reaction of 0,0132 moles of CH₄:
0,0132 mol CH₄× = <em>0,0198 moles</em>
The reaction reaches 77%, moles of Cl₂ that react are: 0,0198×77% = 0,0153 mol
As you have 0,0324 moles of Cl₂, moles that will not react are:
0,0324 - 0,0153 = <em>0,0171 mol Cl₂</em>
As the reaction reaches 77% completion, moles of CH₄ that react are:
0,0132×77% =<em> 0,0102 moles of CH₄ And the moles that don't react are </em><em>0,00300 mol</em>
Thus, moles of each compound are:
0,0102 moles of CH₄×= <em>0,0153 mol + 0,0171 mol = 0,0324 mol Cl₂</em>
0,0102 moles of CH₄×= <em>0,0102 mol CH₄</em>
0,0102 moles of CH₄×= <em>0,0102 mol HCl</em>
0,0102 moles of CH₄×= <em>0,0102 mol Cl⁻</em>
Total pressure using:
P = nRT/V
Where: n = 0,0102mol×3+0,0324mol + 0,0030mol = 0,0660mol; R = 0,082 atmL/molK; T = 298K; V = 2L
Total pressure = 0,806 atm
Partial pressure of CH₄: 0,037 atm
Partial pressure of Cl₂: 0,396 atm
Partial pressure of CH₃Cl: 0,125 atm
Partial pressure of HCl: 0,125 atm
Partial pressure of Cl⁻: 0,125 atm
<em>-To obtain partial pressure you change the moles for each compound-</em>
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I hope it helps!