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lyudmila [28]
3 years ago
6

Where are elements with atomic numbers 1 and 2?

Chemistry
2 answers:
Maru [420]3 years ago
5 0

Answer:hydrogen(H) is 1  and helium(He) is 2

hydrogen is a nonmetal and helium is a nobel gas. hydrogen is found in group S and helium is found in group P

Explanation:hope this helps

rusak2 [61]3 years ago
5 0

Answer:

1 H Hydrogen 1.00797

2 He Helium 4.00260

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At a certain temperature 3.24 moles of co2 gas at 2.15atm takes up a volume of 35.28 what is the temperature in celsius
andrew-mc [135]

Answer:

The temperature is 12.35 C.

Explanation:

An ideal gas is a theoretical gas that is considered to be composed of point particles that move randomly and do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.

An ideal gas is characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them constitutes the ideal gas law, an equation that relates the three variables if the amount of substance, number of moles n, remains constant and where R is the molar constant of the gases:

P * V = n * R * T

In this case:

  • P= 2.15 atm
  • V= 35.28 L
  • n= 3.24 moles
  • R= 0.082 \frac{atm*L}{mol*K}
  • T= ?

Replacing:

2.15 atm* 35.28 L= 3.24 moles* 0.082\frac{atm*L}{mol*K} * T

Solving:

T=\frac{2.15 atm* 35.28 L}{3.24 moles* 0.082\frac{atm*L}{mol*K}}

T=285.5 K= 12.35 C (being 273.15 K= 0 C)

<u><em>The temperature is 12.35 C.</em></u>

3 0
3 years ago
The total volume of hydrogen gas needed to fill the hindenburg was 2.00 × 108 l at 1.00 atm and 25.° c. How much energy was evol
Step2247 [10]

Answer : The energy evolved when it burned was, -2.337\times 10^9KJ

Solution :

First we have to calculate the moles of hydrogen gas by using ideal gas equation.

PV=nRT

where,

P = pressure of gas = 1 atm

V = volume of gas = 2\times 10^8L

T = temperature of gas = 25^oC=273+25=298K

R = gas constant = 0.0821 Latm/moleK

n = number of moles of gas

Now put all the given values in the above formula, we get the moles of hydrogen gas.

(1atm)\times (2\times 10^8L)=n\times (0.0821Latm/moleK)\times (298K)

n=8.174\times 10^6moles

Now we have to calculate the amount of energy evolved.

The combustion reaction of hydrogen will be,

H_2(g)+\frac{1}{2}O_2(g)\rightarrow H_2O(l)

The enthalpy of combustion of hydrogen is -286 KJ/mole. (standard value)

As 1 mole of hydrogen gas burned it evolved energy = -286 KJ

So, 8.174\times 10^6moles of hydrogen gas burned it evolved energy = (8.174\times 10^6)\times (-286)=-2.337\times 10^9KJ

Therefore, the energy evolved when it burned was, -2.337\times 10^9KJ

5 0
3 years ago
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