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sergij07 [2.7K]
3 years ago
11

A 1.2 L weather balloon on the ground has a temperature of 25°C and is at atmospheric pressure (1.0 atm). When it rises to an el

evation where the pressure is 0.71 atm, then the new volume is 1.8 L. What is the temperature (in °C) of the air at this elevation?
Chemistry
1 answer:
natita [175]3 years ago
8 0

Answer: 44.37 degrees C

Explanation:

Use combined gas law: (P1)(V1)/T1=(P2)(V2)/T2

For most gas laws, you  must convert to Kelvin:

K=deg C+273

K=25+273=298 K

Plug and chug:

(1.0 atm)(1.2 L)/(298 K)=(0.71 atm)(1.8 L)/(x)

Solve for x and get 317.37 K

Subtract 273 from this to convert to degrees Celsius. You will get 44.37 degrees Celsius.

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Write a balanced half-reaction describing the oxidation of solid chromium to aqueous chromium(IV) cations.
Pachacha [2.7K]

Answer:

Cr(s) ⟶ Cr⁴⁺(aq) + 4e⁻  

Explanation:

1. Write the skeleton half-reaction

Cr(s) ⟶ Cr⁴⁺(aq)

2. Balance charge

Add electrons to the side that needs them.

You have 4+ on the right and 0 on the left. You must add 4e⁻ to the right to balance the charge.

Cr(s) ⟶ Cr⁴⁺(aq) + 4e⁻

7 0
3 years ago
Describe the motions of particles in the 3 common states of matter
kodGreya [7K]
3 Common States of Matter:

1. Solid - particles are motionless and stick together very closely.

2. Liquid - particles are moving slowly without pattern.

3. Gas - Particles are moving rapidly again without pattern.
3 0
3 years ago
What method is used to removed the unreacted copper (II) carbonate?​
Evgen [1.6K]

Answer:

Filtration

Explanation:

Metal carbonate is insoluble, it is possible to filter off the unreacted substances leaving the desired salt solution

8 0
3 years ago
A gas mixture at 535.0°C and 109 kPa absolute enters a heat exchanger at a rate of 67.0 m3/hr. The gas leaves the heat exchanger
SVEN [57.7K]

Answer:

the heat rate required to cool down the gas from 535°C until 215°C is -2.5 kW.

Explanation:

assuming ideal gas behaviour:

PV=nRT

therefore

P= 109 Kpa= 1.07575 atm

V= 67 m3/hr = 18.6111 L/s

T= 215 °C = 488 K

R = 0.082 atm L /mol K

n = PV/RT = 109 Kpa = 1.07575 atm * 18.611 L/s /(0.082 atm L/mol K * 488 K)

n= 0.5 mol/s

since the changes in kinetic and potencial energy are negligible, the heat required is equal to the enthalpy change of the gas:

Q= n* Δh = 0.5 mol/s * (- 5 kJ/mol) =2.5 kW

7 0
3 years ago
Calculate the molecular weight of a substance. In which the solution of this substance in the water has a concentration of 7 per
Eduardwww [97]

Answer : The molecular weight of a substance is 157.3 g/mol

Explanation :

As we are given that 7 % by weight that means 7 grams of solute present in 100 grams of solution.

Mass of solute = 7 g

Mass of solution = 100 g

Mass of solvent = 100 - 7 = 93 g

Formula used :  

\Delta T_f=i\times K_f\times m\\\\T_f^o-T_f=k_f\times\frac{\text{Mass of substance(solute)}\times 1000}{\text{Molar mass of substance(solute)}\times \text{Mass of water(solvent)}}

where,

\Delta T_f = change in freezing point

T_f^o = temperature of pure water = 0^oC

T_f = temperature of solution = -0.89^oC

K_f = freezing point constant of water = 1.86^oC/m

m = molality

Now put all the given values in this formula, we get

(0-(-0.89))^oC=1.86^oC/m\times \frac{7g\times 1000}{\text{Molar mass of substance(solute)}\times 93g}

\text{Molar mass of substance(solute)}=157.3g/mol

Therefore, the molecular weight of a substance is 157.3 g/mol

7 0
3 years ago
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