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3 years ago

What was one of the first series of event in the study of chemistry

Chemistry

1 answer:

baherus [9]3 years ago

7 0

Discovered and isolated radium and polonium in 1898

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Which statement about subatomic particles is true? (2 points) Protons are the only subatomic particles to have charge. Electrons

Alona [7]

Protons are not the only subatomic particle that has a charge, electrons do to and they are negatively charged. Neutrons are situated in the nucleus of the atom, which means that they do not orbit it. Subatomic particles have different masses.

You are then left with Electrons are the subatomic particles with the smallest mass as your answer.

6 0

3 years ago

A catalyst will

scZoUnD [109]

Answer:

increase the chemical rate

7 0

3 years ago

Help plz I will give u BRAINLIST

Agata [3.3K]

CS2 + 3O2 = CO2 + 2SO2

1 mole of CS2 gives 1 mole of CO2

12 + 2(32) = 76g of CS2 yields 44 g of CO2

Theoretically 1 g of CS2 yields 44/76 g CO2

Therefore 50 g CS2 should yield 50*44 / 76 = 28.95 g

So % yield = 103.6 % ( which is not possible because you can't create matter from nothing).

The 30g cannot be right . This is experimental err.

6 0

3 years ago

Calculate the ΔHrxn for the following

Vesnalui [34]

Answer:

2 NO (g) → N2 (g) + O2 (g)

2 NOCl (g) → 2 NO (g) + Cl2 (g)

____________________________

2NOCl (g) ⟶ N2 (g) + O2 (g) + Cl2 (g)

ΔH = [90.3 kJ x 2 x -1] + [-38.6 kJ x -1 x 2] = -103.4 kJ

The ΔH for the reaction is -103.4 kJ

6 0

3 years ago

What volume (in mL) of a 0.200 MHNO3 solution is required to completely react with 27.6 mL of a 0.100 MNa2CO3 solution according

ladessa [460]

Answer:

There is 27.6 mL of a 0.200 M HNO3 solution required

Explanation:

Step 1: The balanced equation is:

Na2CO3(aq)+2HNO3(aq)→2NaNO3(aq)+CO2(g)+H2O(l)

This means for 1 mole Na2CO3 consumed, there is consumed 2 mole of HNO3 and there is produced 2 moles of NaNO3, 1 mole of CO2 and 1 mole of H2O

Step 2: Calculating moles of Na2CO3

moles of Na2CO3 =volume of Na2CO3 * Molarity of Na2CO3

moles of Na2CO3 = 27.6 *10^-3 * 0.1 M = 0.00276 moles

Step 3: Calculating moles of HNO3

In the balanced equation, we can see that for 1 mole of Na2CO3 consumed, there are consumed 2 moles of HNO3.

So for 0.00276 moles consumed of Na2CO3, there are consumed 0.00552 moles of HNO3.

This means 0.00276 moles of the base Na2CO3 would react with 0.00552 moles of the acid HNO3

Step 4: Calculating the volume of HNO3

volume of HNO3 = moles of HNO3 / Molarity of HNO3

volume of HNO3 = 0.00552 moles / 0.200 M = 0.0276 L

0.0276 L = 27.6 ml

There is 27.6 mL of a 0.200 M HNO3 solution required

4 0

3 years ago