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Paul [167]
3 years ago
9

Describe how the law of conservation of energy is demonstrated in this laboratory activity.

Chemistry
1 answer:
Crank3 years ago
8 0
What laboratory activity. The law of conservation of energy is that energy remains constant. This relates to physics

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If the atoms that share electrons have an unequal attraction for the electrons, the bond is called
VLD [36.1K]

Answer:

A polar covalent bond is a covalent bond in which the atoms have an unequal attraction for electrons and so the sharing is unequal. In a polar covalent bond, sometimes simply called a polar bond, the distribution of electrons around the molecule is no longer symmetrical.

Explanation:

7 0
3 years ago
Which weighs more 10g of iron or 10g of water
Svet_ta [14]

Neither. They are both 10 grams so they weigh the same.

4 0
3 years ago
Read 2 more answers
1.Which of the following are outputs of Cellular Respiration? Choose all that apply *
svlad2 [7]
Oxygen

Photosynthesis 

ATP (chemical energy)
6 0
3 years ago
How many grams of H2O are in 34.2 grams of NAOH<br> Need ASAP
Brrunno [24]

Answer:

15.438g H2O

Explanation:

First you need to find the reaction equation:

2H2O+2Na=2NaOH + H2

Hydrogen is a diatomic molecule so it will have a subscript of 2 on the right hand side. From there we can balance the reaction.    

Then we can use stoichiometry:

34.2g NaOH * (1 mol NaOH/39.908g NaOH) * (2 mol H2O/2 mol NaOH) * (18.015g H2O/1 mol H20) = 15.438g H2O

It is important that when you use stoichiometry that all your units cancel out until you only have the unit you want.

3 0
2 years ago
1) How many molecules are there in 985 mL of nitrogen at 0.0° C and 1.00 x 10-6 mm Hg?
RSB [31]

Answer : The number of molecules present in nitrogen gas are, 3.48\times 10^{13}

Explanation :

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

PV=nRT

where,

P = Pressure of N_2 gas = 1.00\times 10^{-6}mmHg=1.32\times 10^{-9}atm      (1 atm = 760 mmHg)

V = Volume of N_2 gas = 985 mL = 0.982 L    (1 L = 1000 mL)

n = number of moles N_2 = ?

R = Gas constant = 0.0821L.atm/mol.K

T = Temperature of N_2 gas = 0.0^oC=273+0.0=273K

Now put all the given values in above equation, we get:

(1.32\times 10^{-9}atm)\times 0.982L=n\times (0.0821L.atm/mol.K)\times 273K

n=5.78\times 10^{-11}mol

Now we have to calculate the number of molecules present in nitrogen gas.

As we know that 1 mole of substance contains 6.022\times 10^{23} number of molecules.

As, 1 mole of N_2 gas contains 6.022\times 10^{23} number of molecules

So, 5.78\times 10^{-11} mole of N_2 gas contains (5.78\times 10^{-11})\times (6.022\times 10^{23})=3.48\times 10^{13} number of molecules

Therefore, the number of molecules present in nitrogen gas are, 3.48\times 10^{13}

8 0
3 years ago
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