Answer:
40.7062 °C
Explanation:
Let the initial temperature = x °C
Boiling temperature of water = 100 °C
Using,
Q = m C ×ΔT
Where,
Q is the heat absorbed in the temperature change from x °C to 100 °C.
C gas is the specific heat of the water = 4.184 J/g °C
m is the mass of water
ΔT = (100 - x) °C
Given,
Mass = 2350 g
Q = 5.83 × 10⁵ J
Applying the values as:
Q = m C ×ΔT
5.83 × 10⁵ = 2350 × 4.184 × (100 - x)
<u>x, Initial temperature = 40.7062 °C </u>
Answer:
0.1 g/dl
Explanation:
The standard curve is a graph that relates the absorbance at 400 nm with the concentration of haemoglobin in mg/dl. To obtain the concentration from the absorbance value, we enter in the x-axis (absorbance at 400 nm) with the value 0.40 (the line between 0.2 and 0.6), we extrapolate the line to the curve and read the correspondent value on y-axis (concentration in mg/dl): 100 mg/dl.
So, we convert the concentration from mg/dl to g/dl by dividing into 1000:
100 mg/dl x 1 g/1000 mg = 0.1 g/dl
Therefore, the concentration of haemoglobin of the patient is 0.1 g/dl.
Answer:
C. As speed increases, kinetic energy increase exponentially
Explanation:
As you can see on the graph, the further right we move on the x-axis, the higher the values on the y-axis. This means that as one value increases, the other value also increases. The only answer choice that says this is C.
Hope this helps :)
Answer:
Empirical formula: BH3
Molecular Formula: B2H6
Explanation:
To solve the exercise, we need to know how many boron atoms and how many hydrogen atoms the compound has. We know that of the total weight of the compound, 78.14% correspond to boron and 21.86% to hydrogen. As the weight of the compound is between 27 g and 28 g, using the above percentages we can solve that the compound has between 21.1 g and 21.8 g of boron, and between 5.9 g and 6.1 g of hydrogen:
100% _____ 27 g
78.14% _____ x = 78.14% * 27g / 100% = 21.1 g boron
100% ______27 g
21.86% ______ x = 21.86% * 27g / 100% = 5.9 g hydrogen
100% _____ 28 g
78.14% _____ x = 78.14% * 28g / 100% = 21.8 g boron
100% _____ 28g
21.86% _____ x = 21.86% * 28g / 100% = 6.1 g hydrogen
So, if the atomic weight of boron is 10.8 g, there must be two boron atoms in the compound that sum 21.6 g. The weight of hydrogen is 1 g, so the compound must have six hydrogen atoms.
The molecular formula represents the real amount of atoms that form a compound. Therefore, the molecular formula of the compound is B2H6.
The empirical formula is the minimum expression that represents the proportion of atoms in a compound. For example, ethane has 2 carbon atoms and 6 hydrogen atoms, so its molecular formula is C2H6, however, its empirical formula is CH3. Therefore, the empirical formula of the boron compound is BH3.
Heterogeneous mixtures are made of different substances that remain physically seperate. An example would be mixing sand and sugar together.
the answer would be soil
The answer is B soil
