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3 years ago

How do you calculate mass using density and volume?

1 answer:

7 0

Example:

Mass = ?

Density = 25 g/mL

Volume = 5 mL

therefore:

d = m / V

25 = m / 5

m = 25 x 5

m = 125 g

hope this helps!

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30 pts! Sodium and water react according to the following equation. If 31.5g of sodium are added to excess water, how many liter

mihalych1998 [28]

First, calculate the number of moles of sodium present with the given mass,

31.5 g of sodium x (1 mol sodium/ 23 g sodium) = 1.37 mol sodium

It is given in the equation that for every 2mols of sodium, one mol of H2 is produced.

mols of H2 = (1.37 mols sodium)(1 mol H2/ 2 mols sodium)
mols of H2 = 0.685 mols H2

Then, at STP, 1 mol of gas = 22.4 L.

volume of H2 = (0.685 mols H2)(22.4 L / 1 mol)
volume of H2 = 15.34 L

Answer: 15.34 L

3 0

4 years ago

A pressure cooker contains 5.68 liters of air at a temperature of 394 K. If the absolute pressure of the air in the pressure coo

Arturiano [62]

Answer:

Explanation:

We shall find out volume of air at NTP or at 273 K and 10⁵ Pa ( 1 atm )

Let it be V₂

$\frac{P_1V_1}{T_1} =\frac{P_2V_2}{T_2}$

$\frac{2\times 10^5\times 5.68}{394} =\frac{10^5\times V_2}{273}$

V₂ = 7.87 litres

22.4 litres of any gas is equivalent to 1 mole

7.87 litres of air will be equivalent to

7.87 / 22.4 moles

= .35 moles .

7 0

3 years ago

Ammonia is a principal nitrogen fertilizer. It is prepared by the reaction between hydrogen and nitrogen. 3H2(g) + N2(g) → 2NH3(

sergey [27]

Answer:

Explanation:

The equation of the reaction is given as:

3H₂ + N₂ → 2NH₃

Given parameters:

Number of moles of NH₃ = 8moles

Number of moles of H₂ = ?

Number of moles of N₂ = ?

Solution

From the balanced reaction equation, we can establish some mole ratios that would help solve the problem:

To find the number of moles of H₂;

The equation shows that:

2 moles of NH₃ were produced using 3 moles of H₂

therefore: 8 moles of NH₃ will be produced by $\frac{8 x 3}{2}$ = 12moles

So, 12 moles of hydrogen gas will react to give 8 moles of ammonia.

To find the number of moles of N₂

The equation shows that:

2 moles of NH₃ were produced from 1 mole of N₂

8 moles of NH₃ would be produced from $\frac{8 x 1}{2}$ = 4moles of Nitrogen gas

Therefore, 4moles of nitrogen gas would be produced

6 0

3 years ago

Write the name of the first twenty elements with their symbols and their atomic number

7nadin3 [17]

Answer:

1 Hydrogen H

2 Helium He

3 Lithium Li

4 Beryllium Be

5 Boron B

6 Carbon C

7 Nitrogen N

8 Oxygen O

9 Fluorine F

10 Neon Ne

11 Sodium Na

12 Magnesium Mg

13 Aluminium Al

14 Silicon Si

15 Phosphorus P

16 Sulfur S

17 Chlorine Cl

18 Argon Ar

19 Potassium K

20. calcium Ca

6 0

3 years ago

Read 2 more answers

Consider the following exothermic reaction and predict how the change below will affect the concentration (increase, decrease, s

aev [14]

Answer:

a) equilibrium shifts towards the left

b) equilibrium shifts towards the right hand side.

c)equilibrium shifts towards the left hand side

d) addition of argon has no effect on the equilibrium position

e) equilibrium position shifts towards the left hand side

f) equilibrium position is shifted towards the right hand side

g) addition of a catalyst has no effect on the equilibrium position

Explanation:

Given the equation;

3N2H4(g)⇄ 4NH3 (g) + N2 (g)

Adding N2

The addition of N2 will increase the concentration of N2 in the system thereby shifting the equilibrium position to the left in accordance with Le Chatelier's principle.

Removing N2

The removal of N2 drives the forward reaction and the equilibrium shifts towards the right yielding more N2 in accordance with Le Chateliers principle.

Add NH3

The addition of NH3 will shift the equilibrium position towards the left hand side according to Le Chateliers principle.

d) addition of argon has no effect on the equilibrium position.

e) increasing the temperature

Since the reaction is exothermic, increasing the temperature favours the reverse reaction and the equilibrium position his shifted towards the left hand side.

f) Decrease in volume;

Decreasing the volume favours the forward reaction hence the equilibrium position is shifted towards the right.

g) addition of a catalyst has no effect on the equilibrium position.

3 0

3 years ago