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qwelly [4]
2 years ago
13

A certain polyatomic ion contains 49 protons and 50 electrons. What's the net charge of this ion?

Chemistry
1 answer:
timurjin [86]2 years ago
6 0

Explanation:

B more negative charges than positive charges

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2O2 IS THE OXIDIZING AGENT BECAUSE IT GIVES ALL OTHER ELEMENT OXYGEN
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2 years ago
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1) Compared to other main group hydrides, such as CH4, NH3, H2S and HF, water is unique because it is a liquid at room temperatu
ddd [48]
1. d. Water is able to dissolve non-polar gases like oxygen and carbon dioxide.

2. d. -4.8 degree Celsius

3. a. Each solution has the same number of relative particles of solute per kilogram of solvent. 
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3 years ago
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How do you balance the chemical equation NaOH + H2SO4 &gt; Na2SO4 +H2O
jenyasd209 [6]
Make sure there are the same number of atoms of each element on either side.
1) Check each one.
2) If one's out of balance, alter the equation to balance it and go back to 1)
3) When everything's balanced, you're finished!

We have 1 Na on the left and 2 Na on the right here. We'll need another NaOH to balance it:
2 NaOH + H₂SO₄ > Na₂SO₄ + H₂O
Now O is out of balance. There's 6 on the left and 5 on the right. We'll need more H₂O:
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Fortunately H is in balance. S is also in balance here, so looks like we did it!

Need any more help?
5 0
3 years ago
What is a control used for in an experiment?
Setler79 [48]
The control is what you keep the same for each one. For example if you are doing an experiment with plants say you water one with lemon juice, one with milk and one with warm water. The control would be they all have the same amount of sun light and soil. So the growing is equal to keep the experiment fair.
6 0
2 years ago
A chemical factory is making soda ash (NA2CO3) from sodium bicarbonate. The production manager calculates they will make 80 tons
grigory [225]

Answer:

\boxed{\text{ 93 \%}}

Explanation:

\text{\% yield} = \dfrac{\text{actual yield}}{\text {theoretical yield}} \times\text{100 \%}

Data:

\begin{array}{rcr}\text{Actual yield} & = & \text{74.3 T}\\\text{Theoretical yield} & = & \text{80 T}\\\end{array}

Calculation:

\text{\% yield} = \dfrac{\text{74.3 T}}{\text {80 T}} \times\text{100 \%} = \textbf{93 \%}}\\\\\text{The percent yield was } \boxed{\textbf{93 \%}}

7 0
2 years ago
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