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Yanka [14]
2 years ago
9

Help please I really really need it now ​

Chemistry
1 answer:
postnew [5]2 years ago
5 0
1. A 2. B 5. B this is all I know hope it helps
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Find the mass of sodium required to reduce 6.58 L of hydrogen gas at 32°C and 895 mm, when sodium reacts with hydrochloric acid.
Alex

Answer:

Mass = 14.72 g

Explanation:

Given data:

Volume of hydrogen = 6.58 L

Temperature of gas = 32°C (32+273 = 305 k)

Pressure of gas = 895 mmHg (895/760 = 1.2 atm)

Mass of sodium required = ?

Solution:

Chemical equation:

2HCl + 2Na     →      2NaCl + H₂

Number of moles of hydrogen:

PV = nRT

1.2 atm × 6.58 L = n× 0.0821 atm.L/mol.K×305 K

7.9 atm.L =  n×  25.0  atm.L/mol

n = 7.9 atm.L / 25.0  atm.L/mol

n = 0.32 mol

Now we will compare the moles of hydrogen with sodium.

             H₂           :        Na

              1              :        2

            0.32          :     2/1×0.32 = 0.64 mol

Mass of sodium:

Mass = number of moles × molar mass

Mass = 0.64 mol × 23 g/mol

Mass = 14.72 g

3 0
2 years ago
How many neutrons are there in a neutral argon atom? Show how you found your answer on your scratch paper.
mamaluj [8]
There are 22 neutrons in an argon atom. you simply subtract the proton count (atomic number) from the average atomic mass. WORK: 40-18=22
5 0
2 years ago
Calculate the Ka for the following acid. Determine if it is a strong or weak acid. HClO2(aq) dissolves in aqueous solution to fo
Talja [164]

Answer:

The value of Ka = 1.1*10^{-2}

It is a weak  acid

Explanation:

   From the question we are told that

             The concentration of [HClO_2]=0.24M

             The concentration of  [H^+]=0.051M

             The concentration of  [ClO_2^-]=0.051M

Generally the equation for the ionic dissociation of HClO_2 is

                HClO_2_(aq) -------> H^{+}_{(aq)} + ClO_2^{-}_{(aq)}

The equilibrium constant is mathematically represented as

                         Ka = \frac{concentration  \ of  \ product  }{concentration \ of \  reactant }

                               = \frac{[H^+][ClO_2^-]}{[HClO_2]}

Substituting values since all value of concentration are at equilibrium

                    Ka = \frac{0.051 * 0.051}{0.24}

                          = 1.1*10^{-2}

Since the value of  is less than 1 it show that in water it dose not completely

disassociated  so it an acid that is weak

                         

               

3 0
2 years ago
How many grams contained on 78.4 moles of neon
Natali [406]
You have 3.498 moles of the gas/neon
5 0
3 years ago
Read 2 more answers
Calculate the theoretical yield of ammonia produced by the reaction of 100g of H2 gas and 200g of N2 gas
ipn [44]
To get the theoretical yield of ammonia NH3:
first, we should have the balanced equation of the reaction:
3H2(g) + N2(g) → 2NH3(g)
Second, we start to convert mass to moles
moles of N2 = N2 mass / N2 molar mass
                     = 200 / 28 = 7.14 moles
third, we start to compare the molar ratio from the balanced equation between N2 & NH3 we will find that N2: NH3 = 1:2 so when we use every mole of N2 we will get 2 times of that mole of NH3 so,
moles of NH3 = 7.14 * 2 = 14.28 moles 
finally, we convert the moles of NH3 to mass again to get the mass of ammonia:
mass of NH3 = no.moles * molar mass of ammonia
                      = 14.28 * 17 = 242.76 g
6 0
3 years ago
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