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Hoochie [10]
2 years ago
7

How much does 3 moles of silica weigh

Chemistry
1 answer:
amm18122 years ago
6 0

84.2565

Because

1 silica is equal to 28.0855,

times 3 is 84.2565

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Convert 125 g to kilograms
joja [24]
Move the decimal place to the left 3 digits.
0.125
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A student claims that if she wanted to make a solution quickly, she should use small pellets instead of powder along with heatin
vova2212 [387]

Answer: Yes we agree with the student's claim.

Explanation:

When the molecules are present in smaller size, more reactants can react as decreasing the size increases the surface area of the reactants which will enhance the contact of molecules.Hence, more products will form leading to increased rate of reaction.

On increasing the temperature will make more reactant molecules will have sufficient energies to cross the energy barrier and thus the number of effective collisions increases, thus leading to more products and increased rate of reaction.

When the solution is stirred , the molecule's kinetic energy and thus the rate of reaction increases.

Thus smaller size, stirring and increase of temperature will make the solution quickly.

7 0
3 years ago
Calculate the molecular mass or formula mass (in amu) of each of the following substances: (a) BrN3 amu (b) C2H6 amu (c) NF2 amu
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Answer:

Shown below

Explanation:

a) for BrN3

80+3(14)=122amu

b) forC2H6

2(12) + 6(1) = 30amu

C) for NF2

14+2(19) = 52amu

D) Al2S3

2(27) + 3(32)= 150amu

E) for Fe(NO3)3

56 + 3 [14+3(16)] =242amu

F) Mg3N2

3(24) + 2(14)= 100amu

G) for (NH4)2CO3

2[14 +4(1)] +12 +3(16)=96amu

5 0
3 years ago
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If 4.0 g of helium gas occupies a volume of 22.4 L at 0 o C and a pressure of 1.0 atm, what volume does 3.0 g of He occupy under
WINSTONCH [101]

Answer:

the volume occupied by 3.0 g of the gas is 16.8 L.

Explanation:

Given;

initial reacting mass of the helium gas, m₁ = 4.0 g

volume occupied by the helium gas, V = 22.4 L

pressure of the gas, P = 1 .0 atm

temperature of the gas, T = 0⁰C = 273 K

atomic mass of helium gas, M = 4.0 g/mol

initial number of moles of the gas is calculated as follows;

n_1 = \frac{m_1}{M} \\\\n_1 = \frac{4}{4} = 1

The number of moles of the gas when the reacting mass is 3.0 g;

m₂ = 3.0 g

n_2 = \frac{m_2}{M} \\\\n_2 = \frac{3}{4} \\\\n_2 = 0.75 \ mol

The volume of the gas at 0.75 mol is determined using ideal gas law;

PV = nRT

PV = nRT\\\\\frac{V}{n} = \frac{RT}{P} \\\\since, \ \frac{RT}{P} \ is \ constant,\  then;\\\frac{V_1}{n_1} = \frac{V_2}{n_2} \\\\V_2 = \frac{V_1n_2}{n_1} \\\\V_2 = \frac{22.4 \times 0.75}{1} \\\\V_2 = 16.8 \ L

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4 0
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Mars2501 [29]

Answer:

It would increase the final quantity of products

Explanation:

According to the Le- Chatelier principle,

At equilibrium state when stress is applied to the system, the system will behave in such a way to nullify the stress.

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By changing the concentration

By changing the volume

By changing the pressure

By changing the temperature

Consider the following chemical reaction.

Chemical reaction:

2NO₂ ⇄ N₂O₄

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5 0
3 years ago
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