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svlad2 [7]
3 years ago
8

Both renewable and non renewable give us what?

Chemistry
1 answer:
HACTEHA [7]3 years ago
7 0

Answer: Both heat and energy.

Explanation:

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Stella [2.4K]
A neutral atom that loses an electron becomes a positive ion. ... An atom that gains or loses an electron becomes an ion. If it gains a negative electron, it becomes a negative ion. If it loses an electron it becomes a positive ion
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If a reaction is reversible what are the relative amounts of reactant and product
Alina [70]
<span>If a reaction is reversible, then it will attain the phase of Equilibrium and at that phase, the Amount of Reactants and Products would be:  Equal

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Two substances with empirical formula HNO are hyponitrous acid (M = 62.04 g/mol) and nitroxyl (M = 31.02 g/mol).(b) For each spe
Natalija [7]

Below is an attachment of the Lewis structure with the lowest formal charges.

The formal charge is the fictitious charge that an atom in a molecule would have if the electrons in the bonds were evenly distributed among the atoms. The nonbonding electrons on a neutral atom are subtracted from its valence electron count, which is then followed by the number of bonds that bind it to other atoms in the Lewis structure, to get the formal charge. This is another way to put it. When hyponitrous acid is oxidized in the atmosphere, nitric and nitrous acids are produced. By reducing a nitrate or nitrite by sodium amalgam in the presence of water, hyponitrite salts have been created.

Learn more about formal charge here-

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6 0
2 years ago
1. Marisa determined the melting point of a substance to be 24.5C. Find the percent error of her measurement if the actual melti
USPshnik [31]

Answer:

\%\ Error = 21.5\%

Explanation:

Given

Measured = 24.5

Actual = 31.2

Required

Determine the percentage error

First, we need to determine the difference in the measurement

Difference = |Actual - Measured|

Difference = |31.2 - 24.5|

Difference = |6.7|

Difference = 6.7

The percentage error is calculated as thus:

\%\ Error = \frac{Difference * 100\%}{Actual}

\%\ Error = \frac{6.7 * 100\%}{31.2}

\%\ Error = \frac{670\%}{31.2}

\%\ Error = 21.4743589744\%

\%\ Error = 21.5\% <em>approximated</em>

6 0
4 years ago
If a gas has a volume of 1000 ML at a temperature of 23°C and a pressure of 100 mmhg, what is it’s volume under standard conditi
Colt1911 [192]

Answer:

119.7 mL.

Explanation:

  • From the general law of ideal gases:

<em>PV = nRT.</em>

where, P is the pressure of the gas.

V is the volume of the container.

n is the no. of moles of the gas.

R is the general gas constant.

T is the temperature of the gas (K).

  • For the same no. of moles of the gas at two different (P, V, and T):

<em>P₁V₁/T₁ = P₂V₂/T₂.</em>

  • P₁ = 100.0 mmHg, V₁ = 1000.0 mL, T₁ = 23°C + 273 = 296 K.
  • P₂ = 1.0 atm = 760.0 mmHg (standard P), V₂ = ??? mL, T₂ = 0.0°C + 273 = 273.0 K (standard T).

<em>∴ V₂ = (P₁V₁T₂)/(T₁P₂) </em>= (100.0 mmHg)(1000.0 mL)(273.0 K)/(296 K)(760.0 mmHg) =  121.4 <em>mL.</em>

8 0
4 years ago
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