What is the most rare solid

Which of the following bonds is the strongest?

mr Goodwill [35]

The answer to this question will be c

3 0

3 years ago

What scientist do that is the basis

UNO [17]

What does this question mean

5 0

3 years ago

Read 2 more answers

Calculate the volume occupied by 272g

cupoosta [38]

The answer for the following problem is mentioned below.

Therefore volume occupied by methane gas is 184.78 × 10^-3 liters

Explanation:

Given:

mass of methane( $CH_{4}$ ) = 272 grams

pressure (P) = 250 k Pa =250×10^3 Pa

temperature(t) = 54°C =54 + 273 = 327 K

Also given:

R = 8.31JK-1 mol-1 ,

Molar mass of methane( $CH_{4}$ ) = 16.0 grams

We know;

According to the ideal gas equation,

P × V = n × R × T

here,

n = m÷M

n =272 ÷ 16

n = 17 moles

Therefore,

250×10^3 × V = 17 × 8.31 × 327

V = ( 17 × 8.31 × 327 ) ÷ ( 250×10^3 )

V = 184.78 × 10^-3 liters

Therefore volume occupied by methane gas is 184.78 × 10^-3 liters

6 0

3 years ago

For the reaction N2(g) + 2H2(g) → N2H4(l), if the percent yield for this reaction is 100.0%, what is the actual mass of hydrazin

barxatty [35]

Answer:

53.6 g of N₂H₄

Explanation:

The begining is in the reaction:

N₂(g) + 2H₂(g) → N₂H₄(l)

We determine the moles of each reactant:

59.20 g / 28.01 g/mol = 2.11 moles of nitrogen

6.750 g / 2.016 g/mol = 3.35 moles of H₂

1 mol of N₂ react to 2 moles of H₂

Our 2.11 moles of N₂ may react to (2.11 . 2) /1 = 4.22 moles of H₂, but we only have 3.35 moles. The hydrogen is the limiting reactant.

2 moles of H₂ produce at 100 % yield, 1 mol of hydrazine

Then, 3.35 moles, may produce (3.35 . 1)/2 = 1.67 moles of N₂H₄

Let's convert the moles to mass:

1.67 mol . 32.05 g/mol = 53.6 g

4 0

3 years ago

The pressure inside a compressed gas cylinder is 144 atm at 48°C. What will the pressure inside the cylinder be after it is cool

Andrews [41]

<h3>Answer:</h3>

134 atm

<h3>Explanation:</h3>

Based on the pressure law, the pressure of a gas varies directly proportionally to the absolute temperature at a constant volume.

Therefore; we are going to use the equation;

$\frac{P1}{T1}=\frac{P2}{T2}$

In this case;

Initial pressure, P1 = 144 atm

Initial temperature, T1 (48°C) = 321 K

Final temperature, T2 (25°C) = 298 K

We need to find the final pressure,

Therefore;

P2 = (P1/T1)T2

= (144/321)× 298 K

= 133.68 atm

= 134 atm

Therefore, the new pressure will be 134 atm.

5 0

4 years ago