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3 years ago

The greater the resistance, the less current there is for a given voltage. True or False

Chemistry

2 answers:

USPshnik [31]3 years ago

8 0

Your answer will be True because without the resistance it can not make a voltage.

Your answer is True.

mart [117]3 years ago

7 0

True the answer is true

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Fe2O3(s) + 3CO(g) ---> 2Fe(l) + 3CO2(g) Steve inserts 450. g of iron(III) oxide and 260. g of carbon monoxide into the blast

baherus [9]

Answer: Theoretical yield is 313.6 g and the percent yield is, 91.8%

Explanation:

To calculate the moles :

$\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}$

$\text{Moles of} Fe_2O_3=\frac{450}{160}=2.8moles$

$\text{Moles of} CO=\frac{260}{28}=9.3moles$

$Fe_2O_3(s)+3CO(g)\rightarrow 2Fe(l)+3CO_2(g)$

According to stoichiometry :

1 mole of $Fe_2O_3$ require 3 moles of $CO$

Thus 2.8 moles of $Fe_2O_3$ will require= $\frac{3}{1}\times 2.8=8.4moles$ of $CO$

Thus $Fe_2O_3$ is the limiting reagent as it limits the formation of product and $CO$ is the excess reagent.

As 1 mole of $Fe_2O_3$ give = 2 moles of $Fe$

Thus 2.8 moles of $Fe_2O_3$ give = $\frac{2}{1}\times 2.8=5.6moles$ of $Fe$

Mass of $Fe=moles\times {\text {Molar mass}}=2.6moles\times 56g/mol=313.6g$

Theoretical yield of liquid iron = 313.6 g

Experimental yield = 288 g

Now we have to calculate the percent yield

$\%\text{ yield}=\frac{\text{Actual yield }}{\text{Theoretical yield}}\times 100=\frac{288g}{313.6g}\times 100=91.8\%$

Therefore, the percent yield is, 91.8%

6 0

3 years ago

What is the volume, in liters, of 4.00 moles of methane gas, CH4, at 13 ∘C and 1.20 atm?

dimulka [17.4K]

Answer:

78.268L

Signifigant figures = 78L

6 0

3 years ago

What is true of an Arrhenius acid?

expeople1 [14]

<span>B, An Arrhenius acid donates H+ ions.</span>

5 0

3 years ago

What is the weight of oxygen in 50gwater

8_murik_8 [283]

To compute the required mass of the element to form the given molecules, we'll use the general formula shown below:

{eq}\displaystyle m_1=\frac{M_1}{M_2}\times m_2 {/eq}, where,

{eq}M_1 {/eq} is the molecular weight of the element.

{eq}M_2 {/eq} is the molecular weight of the given molecule.

{eq}m_2 {/eq} is the mass of the given molecule.

Answer and Explanation:

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The given value is:

The value of the mass of the water molecule is {eq}m_2=\rm 50\ grams {/eq}.

The chemical reaction for the formation of water...

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Formula for Mass: Definition & Examples

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Chapter 28 / Lesson 42

52K

What is mass? Learn the mass definition and how to find the mass of an object using the mass formula. See common mass characteristics and properties.

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5 0

2 years ago

The terms Q and K refer to reaction components at non-equilibrium and equilibrium conditions, respectively. For a forward reacti

daser333 [38]

Answer:

The value of Q must be less than that of K.

Explanation:

The difference of K and Q can be understood with the help of an example as follows

A ⇄ B

In this reaction A is converted into B but after some A is converted , forward reaction stops At this point , let equilibrium concentration of B be [B] and let equilibrium concentration of A be [A]

In this case ratio of [B] and [A] that is

K = [B] / [A] which is called equilibrium constant.

But if we measure the concentration of A and B ,before equilibrium is reached , then the ratio of the concentration of A and B will be called Q. As reaction continues concentration of A increases and concentration of B decreases. Hence Q tends to be equal to K.

Q = [B] / [A] . It is clear that Q < K before equilibrium.

If Q < K , reaction will proceed towards equilibrium or forward reaction will

proceed .

8 0

3 years ago