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xxMikexx [17]
3 years ago
7

36 g of water vapor takes up how many liters at room temperature and pressure of 293K and 100 K PA

Chemistry
2 answers:
qaws [65]3 years ago
7 0

Answer:-

48.72 L

Explanation:-

Chemical formula of water= H2O

Mass of water = 36 g

Molar mass of water = 1 x 2 + 16 x 1 = 18 g mol-1

Number of moles of water = n = 36 g / (18 g mol-1)

= 2 moles.

Temperature T = 293 K

Pressure = P = 100 K Pa

Universal gas constant R = 8.314 L KPa K -1 mol-1

Using the relation PV = nRT

we get Volume V = nRT/P

Plugging in the values

V = (2 moles ) x ( 8.314 L KPa K -1 mol-1) x ( 293 K) / 100 K Pa

= 48.72 L

crimeas [40]3 years ago
6 0

100kpa is correct .100 kpa is correct

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Answer:

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I HOPE MY ANSWER WILL HELP YOU :)

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Determine the frequency of light with a wavelength of 2.672 x 10^-7cm
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What feature forms on the ocean floor at a divergent plate boundary where two pieces of oceanic crust are moving away from each
solong [7]

Answer:

volcanos i think

Explanation:

learned it in 6th grade

6 0
3 years ago
A piece of wood near a fire is at 23°c. it gains 1,160 joules of heat from the fire and reaches a temperature of 42°c. the speci
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The mass of the piece of wood is 35.58 g.

Joule = M × T × C

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Substituting the values in the equation,

1160 = M × 19 × 1.716

M = 1160/32.604 = 35.58 g

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<h3>What is meant by specific heat capacity?</h3>

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7 0
1 year ago
onsider the reaction, NO2(g) + CO(g) → NO(g) + CO2(g), for which the rate law has been determined to be: Rate = k[NO2]2[CO]. Whi
nlexa [21]

Answer:

The correct answer is option D.

Explanation:

Rate of the reaction is a change in the concentration of any one of the reactant or product per unit time.

NO_2(g) + CO(g)\rightarrow NO(g) + CO_2(g)

Rate of the reaction:

R=-\frac{1}{1}\times \frac{d[NO_2]}{dt}=-\frac{1}{1}\times \frac{d[CO]}{dt}

Rate of decrease in nitrogen dioxide concentration is equal to the rate of decrease in carbon monoxide.

Given rate expression of the reaction:

R = k[NO2]^2[CO]

Rate of the reaction on doubling concentration of nitrogen dioxide and carbon monoxide : R'

R'=k(2\times [NO_2])^2(2\times [CO])=8\times k[NO2]^2[CO]=8R

Doubling the concentrations of nitrogen dioxide and carbon monoxide simultaneously will increase the rate of the reaction by a factor of eight.

Hence, none of the given statements are true.

6 0
3 years ago
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