All categories

3 years ago

How many moles of CO2 are in 1.0L at 25 degrees C and 95 kPa?

1 answer:

5 0

The problem with this is which R do you use in PV = nRT. Everything else is straightforward. You can google the multitude of Rs that come about because the only difference is in the units used. Most of the time it is 8.314. When you google, call it the gas constant in PV = nRT. Keep it bookmarked when you are doing problems in this section.

R = 8.314 L kPa/(mol oK)
T = 25oC = 25 + 273 = 298oK
P = 95000 Pa
V = 1.0 L

Now you are all set to find n
Rearrange the formula
n = PV/(RT)
n = 95000 * 1/ (8.314 * 298)
n = 38.343 Seems like an awful lot. But that's what you are getting

You might be interested in

A 0.200 M solution of a weak acid, HA, is 9.4% ionized. Using this information, calculate Ka for HA.

slavikrds [6]

${ \qquad\qquad\huge\underline{{\sf Answer}}}$

Let's solve ~

Initial concentration of weak acid HA = 0.200 M

and dissociation constant ( ${ \alpha}$ ) is :

$\qquad \sf \dashrightarrow \: \alpha = \frac{dissociation \: \: percentage}{100}$

$\qquad \sf \dashrightarrow \: \alpha = \frac{9.4}{100} = 0.094$

Now, at initial stage :

$\textsf{ Conc of HA = 0.200 M}$

$\textsf{Conc of H+ = 0 M}$

$\textsf{Conc of A - = 0 M}$

At equilibrium :

$\textsf{Conc of HA = 0.200 - 0.094(0.200) = 0.200(1 - 0.094) = 0.200(0.906) = 0.1812 M}$

$\textsf{Conc of H+ = 0.094(0.200) = 0.0188 M}$

$\textsf{Conc of A - = 0.094(0.200) = 0.0188 M}$

Now, we know :

$\qquad \sf \dashrightarrow \: { K_a = \dfrac{[H+] [A-]}{[HA]}}$

( big brackets represents concentration )

$\qquad \sf \dashrightarrow \: { K_a = \dfrac{0.0188×0.0188}{0.1812}}$

$\qquad \sf \dashrightarrow \: { K_a = \dfrac{0.00035344}{0.1812}}$

$\qquad \sf \dashrightarrow \: { K_a \approx 0.00195 }$

$\qquad \sf \dashrightarrow \: {K_a \approx 1.9 × {10}^{-3} }$

7 0

2 years ago

Complete the passage to describe how electrons are represented in electron dot diagrams. The maximum number of dots an electron

romanna [79]

D. 8, A. 2

Hope this helps

6 0

4 years ago

Read 2 more answers

Sue has to find the empirical formula of a compound containing 81.8 grams of carbon and 18.2 grams of hydrogen in 100 grams of c

ArbitrLikvidat [17]

She would divide that mass of each element by it molar mass the answer is C <span />

6 0

3 years ago

How much heat (kj) is required to convert 3.12 moles of liquid benzene at 75.1Â°c to gaseous benzene at 115.1Â°c?

Tems11 [23]

The total energy includes sensible heat to raise the temperature from 75.1°C to the boiling point. It also includes the latent heat to convert the liquid to gas. Then, it also includes sensible heat from he boiling point to 115.1°C. The equation is:

Energy = nCp,liquid(T,bp - T₁) + nΔH + nCp,gas(T₂ - T,bp)
where
n is the number of moles
T,bp is the boiling point of benzene at 80.1°C
Cp,liquid = 134.8 J/mol·°C
Cp,gas = 82.44 J/mol·°C
ΔH = 87.1 J/mol

Energy = (3.12 moles)(134.8 J/mol·°C)(80.1°C - 75.1°C) + (3.12 moles)(87.1 J/mol) + (3.12 moles)(82.44 J/mol·°C)(115.1°C - 80.1°C)
Energy = 11,377.08 J

3 0

3 years ago

Why does the earth experience unequal heating

evablogger [386]

Global Warming is tthe cause

3 0

3 years ago