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2 years ago

If the volume of a container of gas is reduced, what will happen to the pressure inside the container?

Chemistry

2 answers:

blondinia [14]2 years ago

8 0

B).The pressure will not change

andrew11 [14]2 years ago

5 0

Answer: a. The pressure will increase.

Explanation:

Boyle's Law: This law states that pressure is inversely proportional to the volume of the gas at constant temperature and number of moles.

$P\propto \frac{1}{V}$ (At constant temperature and number of moles)

${P_1V_1}={P_2V_2}$

where,

$P_1$ = initial pressure of gas

$P_2$ = final pressure of gas

$V_1$ = initial volume of gas

$V_2$ = final volume of gas

Thus as volume of the container will be reduced, the pressure would increase.

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__ P4(s) + __ O2(g) → __ P4O10(s) Now we will balance O. How many O2 molecules are needed to form one P4O10 molecule?

Mnenie [13.5K]

Answer:

Five molecules of oxygen.

Explanation:

Hello,

In this case, considering the given chemical reaction, we must write a five before the oxygen in order to equal the number of oxygen atoms at both the right and left side (ten) so phosphorous remain the same (4):

$P_4(s) + 5 O_2(g)\rightarrow P_4O_{10}(s)$

It means that five molecules of oxygen (O₂) are needed to form one molecule of tetraphosphorous decaoxide (P₄O₁₀).

Best regards.

4 0

2 years ago

What volume of 0.500 M HNO₃(aq) must completely react to neutralize 100.0 milliliters of 0.100 M KOH(aq)?

USPshnik [31]

Answer:

v = 500 milliliters

Explanation:

$HNO_{3}$ ⇒ $H^{+} + NO^{3-}$

$KOH$ ⇒ $K^{+} + OH^{-}$

1 $H^{+}$ to 1 $OH^{-}$

$\frac{0,5}{V} = \frac{0,1}{100} \\\\v * 0,1 = 50\\v = 500 milliliters$

4 0

2 years ago

The Mond process produces pure nickel metal via the thermal decomposition of nickel tetracarbonyl: Ni(CO)4 (l) → Ni (s) + 4CO (g

Yuki888 [10]

<u>Answer:</u> The volume of CO formed is 254.43 L.

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Given mass of $Ni(CO)_4$ = 444 g

Molar mass of $Ni(CO)_4$ = 170.73 g/mol

Putting values in above equation, we get:

$\text{Moles of }Ni(CO)_4=\frac{444g}{170.73g/mol}=2.60mol$

For the given chemical reaction:

$Ni(CO)_4(l)\rightarrow Ni(s)+4CO(g)$

By stoichiometry of the reaction:

1 mole of nickel tetracarbonyl produces 4 moles of carbon monoxide.

So, 2.60 moles of nickel tetracarbonyl will produce = $\frac{4}{1}\times 2.60=10.4mol$ of carbon monoxide.

Now, to calculate the volume of the gas, we use ideal gas equation, which is:

PV = nRT

where,

P = Pressure of the gas = 752 torr

V = Volume of the gas = ? L

n = Number of moles of gas = 10.4 mol

R = Gas constant = $62.364\text{ L Torr }mol^{-1}K^{-1}$

T = Temperature of the gas = $22^oC=(273+22)K=295K$

Putting values in above equation, we get:

$752torr\times V=10.4mol\times 62.364\text{ L Torr }mol^{-1}K^{-1}\times 295K\\\\V=254.43L$

Hence, the volume of CO formed is 254.43 L.

5 0

2 years ago

Round off each of the following numbers to two significant figures:

Kay [80]

A) 5.2 x 10^2
B) 86.
C) 6.4 x 10^3
D) 5.0
E) 22.
F) 0.89

7 0

2 years ago

Read 2 more answers

A 2.40 kg block of ice is heated with 5820 J of heat. The specific heat of water is 4.18 J•g^-1•C^-1. By how much will it’s temp

MrMuchimi

Answer: The temperature rise is $0.53^0C$

Explanation:

The quantity of heat required to raise the temperature of a substance by one degree Celsius is called the specific heat capacity.

$Q=m\times c\times \Delta T$

Q = Heat absorbed by ice = 5280 J

m = mass of ice = 2.40 kg = 2400 g (1kg=1000g)

c = heat capacity of water = $4.18J/g^0C$

Initial temperature = $T_i$

Final temperature = $T_f$

Change in temperature , $\Delta T=T_f-T_i=?$

Putting in the values, we get:

$5280J=2400g\times 4.18J/g^0C\times \Delta T$

$\Delta T=0.53^0C$

Thus the temperature rise is $0.53^0C$

0 0

2 years ago