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4 years ago

12

The lower the ignition temperature, better the fuel. True or false?Why?

1 answer:

Aleksandr [31]4 years ago

3 0

Answer:

True

Explanation:

This means the fuel is highly flammable hence it has a low ignition temperature. This, therefore, means it burns fast without putting in a lot of energy to ignite it. Even in cars, therefore, the compression ratios, in engines using these of these fuels, is lesser.

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I need help with this guys

Flura [38]

I have no idea I’m answering this because I need to ask more questions

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3 years ago

As you move from row ______ to row ______ in the periodic table, the atomic radius of the elements DECREASES.

Len [333]

Answer:

C) 7 to 1

Explanation:

The periodic trend of Atomic Radii for the Periodic Table of Elements is down and to the left the atomic radii increases.

So, from period 1 to 7 and group 18 to group 1, the atomic radii increases.

The opposite (decreasing) would be from period 7 to 1 and group 1 to group 18.

Therefore, our answer is C.

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3 years ago

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Nat2105 [25]

Answer:

either element or pure substance but i think its element

Explanation:

7 0

3 years ago

Read 2 more answers

Liquid hydrogen boils at -252°C. What is the boiling point on the Kelvin scale?

DaniilM [7]

Answer:

Boiling point in kelvin is 373.1 \

boiling point of liquid hydrogen in kelvin is 21.15

Explanation:

5 0

3 years ago

A chemistry graduate student is given 125.mL of a 0.20M acetic acid HCH3CO2 solution. Acetic acid is a weak acid with =Ka×1.810−

Over [174]

Answer : The mass of sodium acetate is, 1.097 grams.

Explanation : Given,

The dissociation constant for acetic acid = $K_a=1.8\times 10^{-5}$

Concentration of acetic acid (weak acid)= 0.20 M

volume of solution = 125. mL

pH = 4.47

First we have to calculate the value of $pK_a$ .

The expression used for the calculation of $pK_a$ is,

$pK_a=-\log (K_a)$

Now put the value of $K_a$ in this expression, we get:

$pK_a=-\log (1.8\times 10^{-5})$

$pK_a=5-\log (1.8)$

$pK_a=4.74$

Now we have to calculate the concentration of sodium acetate (conjugate base or salt).

Using Henderson Hesselbach equation :

$pH=pK_a+\log \frac{[Salt]}{[Acid]}$

Now put all the given values in this expression, we get:

$4.47=4.74+\log (\frac{[Salt]}{0.20})$

$[Salt]=0.107M$

Now we have to calculate the mass of sodium acetate.

$\text{Concentration}=\frac{\text{Mass of }NaCH_3CO_2\times 1000}{\text{Molar mass of }NaCH_3CO_2\times \text{Volume of solution (in mL)}}$

$0.107M=\frac{\text{Mass of }NaCH_3CO_2\times 1000}{82g/mol\times 125mL}$

$\text{Mass of }NaCH_3CO_2=1.097g$

Therefore, the mass of sodium acetate is, 1.097 grams.

6 0

4 years ago