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sattari [20]
4 years ago
10

Which of the following is a testable hypothesis

Chemistry
1 answer:
natka813 [3]4 years ago
8 0

Answer:

C

Explanation:

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Determine the oxidation state of nitrogen in lino3.
Andre45 [30]

Answer : The oxidation state of nitrogen in LiNO_3 is, (+5)

Explanation :

Rules for the oxidation numbers :

  • The oxidation number of a free element is always be zero.
  • The oxidation number of a monatomic ion equal to the charge of the ion.
  • The oxidation number of  Hydrogen (H)  is +1.
  • The oxidation number of  oxygen (O)  in compounds is usually -2, but it is -1 in the peroxides.
  • The oxidation number of a Group 1 element in a compound is +1.
  • The oxidation number of a Group 2 element in a compound is +2.
  • The oxidation number of a Group 17 element in a binary compound is -1.
  • The sum of the oxidation numbers of all of the atoms in a neutral compound is zero.
  • The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion.

The given compound is, LiNO_3

Let the oxidation state of 'N' be, 'x'

(+1)+x+3(-2)=0\\\\x=+5

Hence, the oxidation state of N is, (+5)

3 0
4 years ago
Read 2 more answers
What dos the line of red semicircles maen on the weather map
PIT_PIT [208]
The red semicircle shown in the weather chart represents warm front.

6 0
4 years ago
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6.0 L of gas in a piston at a pressure of 1.0 atm are compressed until the volume is 3.5 L. What is the new pressure inside the
dimulka [17.4K]

From the calculations and by the use of Boyles law, the new pressure of the gas is 1.7 atm

<h3>What are gas laws?</h3>

The term gas law is used to demonstrate the relationship between the volume, pressure, number of moles and temperature of a gas.

Using the Boyles law;

P1 = 1 atm

P2 = ?

V1 = 6 L

V2 = 3.5 L

P1V1= P2V2

P2= P1V1/V2

P2= 1 atm * 6 L/3.5 L

= 1.7 atm

Learn more about Boyles law:brainly.com/question/1437490

#SPJ1

3 0
2 years ago
Of the following gases, ________ will have the greatest rate of effusion at a given temperature. Of the following gases, _______
kolezko [41]

<u>Answer:</u> From the given gases, the greatest rate of effusion is of CH_4

<u>Explanation:</u>

Rate of effusion of a gas is determined by a law known as Graham's Law.

This law states that the rate of effusion or diffusion of a gas is inversely proportional to the square root of the molar mass of the gas. The equation given by this law follows:

\text{Rate of diffusion}\propto \frac{1}{\sqrt{\text{Molar mass of the gas}}}

It is visible that molar mass is inversely related to rate of effusion. So, the gas having lowest molar mass will have the highest rate of effusion.

For the given gases:

Molar mass of NH_3=17g/mol

Molar mass of HCl=36.5g/mol

Molar mass of CH_4=16g/mol

Molar mass of Ar=40g/mol

Molar mass of HBr=81g/mol

The molar mass of methane gas is the lowest. Thus, it will have the greatest rate of effusion.

Hence, the greatest rate of effusion is of CH_4

8 0
4 years ago
Is this equation balanced or unbalanced?<br> C+02=CO2
LenKa [72]
This equation is balanced
4 0
3 years ago
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