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shusha [124]
3 years ago
9

If the pressure of a gas is 1.01 atm and the temperature is 25°C, then if the pressure is increased to 1.10, what is the new tem

perature?
Chemistry
1 answer:
vodka [1.7K]3 years ago
3 0

Answer:

T2 = 51.6°C

Explanation:

Given:

P1 = 1.01 atm

T1 = 25°C + 273 = 298K

P2 = 1.10 atm

T2 = ?

P1/T1 = P2/T2

Solving for T2,

T2 = (P2/P1)T1

= (1.10 atm/1.01 atm)(298K)

= 324.6 K

= 51.6°C

where Tc = Tk - 273

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Consider the following reaction: NaHCO3 + HC2H3O2 → NaC2H3O2 + H2O + CO2 How many g of CO2 would be produced from the complete r
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<h2>1.25 g of CO_2 would be produced from the complete reaction of 25 mL of 0.833 mol/L HC_3H_3O_2 with excess NaHCO_3 </h2>

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\text{Molarity of the solution}=\frac{\text{Moles of solute}\times 1000}{\text{Volume of solution (in L)}}    

0.833M=\frac{\text{Moles of} HC_3H_3O_2\times 1000}{25ml}\\\\\text{Moles of} HC_3H_3O_2 =\frac{0.833mol/L\times 25}{1000}=0.0208mol

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According to stoichiometry:

1 mole of HC_2H_3O_2 will give = 1 mole of CO_2

0.0208 moles of HC_2H_3O_2 will give =\frac{1}{1}\times 0.0208=0.0208 moles of CO_2

Mass of HC_2H_3O_2=moles\times {\text {molar mass}}=0.0208\times 60g/mol=1.25g

Thus 1.25 g of CO_2 would be produced from the complete reaction of 25 mL of 0.833 mol/L HC_3H_3O_2 with excess NaHCO_3

Learn more about molarity

https://brainly.in/question/13034158

#learnwithbrainly

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