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anyanavicka [17]

2 years ago

9

a volumetric pipette haas an uncertainty of 0.01 cm what are the lowest and highest possible volumes for a measurement of 0.20cm

1 answer:

Vanyuwa [196]2 years ago

5 0

Answer:

Possible lowest volume = 0.19 cm

Possible highest volume = 0.21 cm

Explanation:

Given Data

uncertainty = 0.01 cm

total volume = 0.20 cm

Possible lowest volume = ?

Possible highest volume = ?

Solution:

Possible lowest volume = total volume - uncertainty

Possible lowest volume = 0.20 cm - 0.01 cm

Possible lowest volume = 0.19 cm

Possible highest volume = total volume + uncertainty

Possible highest volume = 0.20 cm - 0.01 cm

Possible highest volume = 0.21 cm

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The following reaction shows the process of rusting. 4Fe + 3O2= 2Fe2O3 This chemical reaction should be classified as _____.

andrezito [222]

This is a synthesis reaction, where 2 reactants combine to form a single product.

In decomposition, 1 reactant splits into 2 products.
In single replacement, one element swaps with another, in the form A + BC = B + AC.
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In neutralization (a kind of double displacement), an acid and a base react to form water and a salt.

5 0

3 years ago

Read 2 more answers

Volume increases, pressure stays the same, temperature

Mila [183]

Temperature decreases (?)

4 0

2 years ago

2C2H2 + 5O2 → 4CO2 + 2 H2O How many grams of CO2 are required to react with exactly 3.00 mol of O2? 106 g 132 g 165 g 76.8 g

cricket20 [7]

Hey there!:

Given the reaction:

2 C2H2 + 5 O2 → 4 CO2 + 2 H2O

5 moles O2 ------------- 4 moles CO2

3.00 moles O2 ---------- ( moles of CO2 ?? )

moles of CO2 = 3.00 * 4 / 5

moles of CO2 = 12 / 5

moles of CO2 = 2.4 moles

So, molar mass CO2 = 44.01 g/mol

Therefore:

1 mole CO2 -------------- 44.01 g

2.4 moles CO2 ---------- ( mass of CO2 )

mass of CO2 = 2.4 * 44.01 / 1

mass of CO2 = 106 g

Answer A

Hope that helps!

8 0

3 years ago

g If 50.0 mL of a 0.75 M acetic acid solution is titrated with 1.0 M sodium hydroxide, what is the pH after 10.0 mL of NaOH have

V125BC [204]

Answer:

pH = 2.66

Explanation:

Acetic Acid + NaOH → Sodium Acetate + H₂O

First we <u>calculate the number of moles of each reactant</u>, using the <em>given volumes and concentrations</em>:

0.75 M Acetic acid * 50.0 mL = 37.5 mmol acetic acid

1.0 M NaOH * 10.0 mL = 10 mmol NaOH

We<u> calculate how many acetic acid moles remain after the reaction</u>:

37.5 mmol - 10 mmol = 27.5 mmol acetic acid

We now <u>calculate the molar concentration of acetic acid after the reaction</u>:

27.5 mmol / (50.0 mL + 10.0 mL) = 0.458 M

Then we <u>calculate [H⁺]</u>, using the<em> following formula for weak acid solutions</em>:

[H⁺] = $\sqrt{C*Ka}=\sqrt{0.458M*1.76x10^{-5}}$

[H⁺] = 0.0028

Finally we <u>calculate the pH</u>:

pH = -log[H⁺]

pH = 2.66

8 0

2 years ago

For many purposes we can treat ammonia NH3 as an ideal gas at temperatures above its boiling point of −33.°C. Suppose the temper

Keith_Richards [23]

Answer:

The new pressure will be 0.225 kPa.

Explanation:

Applying combined gas law:

$\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}$

where,

$P_1\text{ and }V_1$ are initial pressure and volume at initial temperature $T_1$ .

$P_2\text{ and }V_2$ are final pressure and volume at initial temperature $T_2$ .

We are given:

$P_1=0.29 kPa\\V_1=V\\P_2=?\\V_2=V+50\% of V=1.5 V$

$T_1=-25^oC=248.15 K$

$T _2 = 16^oC=289.15 K$

Putting values in above equation, we get:

$\frac{0.29 kPa\times V}{248.15 K}=\frac{P_2\times 1.5V}{289.15 K}$

$P_1=0.225 kPa$

Hence, the new pressure will be 0.225 kPa.

4 0

3 years ago